1. History of Chemistry

2. The Greeks 4 elements: - Fire: Hot & Dry - Earth: Dry & Cold
- Water: Cold & Wet
- Air: Wet & Hot

3. The Alchemists “Fake Scientists” Tried to turn cheap metals into gold
Discovered elements such as mercury and sulfur
“The Chymist”

4. “The First Chemist” Robert Boyle (1627-1691)
Science should be firmly grounded in experiments.
An element is something that cannot be broken down into simpler substances.
There are probably many elements.

5. II. Elements

6. A. Abundant Pure Elements in the Atmosphere
Nitrogen
Oxygen
Argon

7. B. Abundant Elements (By Mass)
Human Body
Earth’s Atmosphere
Earth’s Oceans
Earth’s Crust
O (65)
C (18)
H (10)
N (3)
Ca (1.5)
P (1.2)
Others
N (78.1)
O (20.9)
Ar (0.96) C H
O (85.8)
H (10.8)
Cl (1.9)
Na (1.1) Others (0.4)
Sorry, oil. Lots and lots of oil.
O (46.6)
Si (27.7)
Al (8.1)
Fe (5)
Ca (3.6)
Na (2.8)

8. C. Trace Elements Copper - production of red blood cells
Elements that your body needs, but only in small amounts.
Examples:
Copper - production of red blood cells
Iodine - functioning of thyroid gland
Chromium - metabolism of sugars

9. III. Laws of Matter

10. A. Law of Conservation of Mass
Mass can neither be created nor destroyed

11. B. Law of Definite Proportion (constant composition)
A given compound always contains exactly the same proportion of elements by mass
NaCl: 39.3% Na; 60.7% Cl
H2O: 11.1% H; 88.9% O

12. C. Law of Multiple Proportions
When 2 elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to whole numbers.
Example:
H2O * H2O2
1 gram H, 8 grams O 1 gram H, 16 grams O

13. The Atom John Dalton (1766-1844)
Dalton’s Atomic Theory
Elements are made of tiny particles called atoms.
All atoms of a given element are identical.
The atoms of a given element are different from those of any other element.
Atoms of one element can combine with atoms of other elements to form compounds. A given compound always has the same relative numbers and types of atoms.

14. The Atom John Dalton (1766-1844)
Dalton’s Atomic Theory
5. Atoms are indivisible in chemical processes. That is, atoms are not created or destroyed in chemical reactions. A chemical reaction simply changes the way atoms are grouped together.

15. The Atom J.J. Thomson ( )
Discovered electrons using the cathode ray tube experiment
With Lord Kelvin, he believed that the negative electrons were stuck in a positive sphere (Plum pudding model)

16. Cathode Ray Tube

17. The Atom Robert Millikan (1909)
Calculated the charge (-1.6 x Coulombs) and mass of an electron using the oil drop experiment

18. The Atom Ernest Rutherford (1871-1937)
Discovered the positively charged nucleus using the gold foil experiment.
(The atom was mostly empty space, with a dense, positive center.)

19. The Atom Gold Foil Experiment

20.                               
The Atom Niels Bohr (1913)
Believed that electrons moved around the nucleus in rings or shells like planets around the sun
(Solar System Model)

21. The Atom James Chadwick (1932)
                              
The Atom James Chadwick (1932)
Discovered the neutron

22. The Atom Quantum Mechanical Model
                              
The Atom Quantum Mechanical Model
Electrons exist in orbitals around the nucleus.

23. Sources www.chemheritage.org www.aip.org/history
“The Chymist” by David Teniers